pH, Salts and their Uses

50 lessons, pages 1251–1300.

  1. Acids, Bases and Salts as a Connected System — Relating proton transfer, aqueous ions and neutralisation products
  2. Acid Behavior in Water — Hydronium formation and the limits of the hydrogen-ion shorthand
  3. Base Behavior in Water — Hydroxide release and proton acceptance by dissolved bases
  4. Conjugate Acid–Base Pairs — Tracking one transferred proton across an equation
  5. Water as an Acid and a Base — Amphiprotic behavior in opposite proton-transfer reactions
  6. Strong and Weak Acids — Extent of ionisation rather than concentration or danger
  7. Strong and Weak Bases — Dissociation and proton-acceptance equilibria in water
  8. Concentration Versus Acid Strength — Separating the amount dissolved from the fraction ionised
  9. The Self-Ionisation of Water — Hydronium and hydroxide in pure water
  10. Ion-Product Constant of Water — Using Kw at a stated temperature
  11. The Meaning of pH — A logarithmic measure linked to hydronium activity
  12. Calculating pH from Hydronium Concentration — Introductory dilute-solution calculations with powers of ten
  13. Finding Hydronium Concentration from pH — Reversing the base-ten logarithm
  14. The Meaning of pOH — Expressing hydroxide concentration on a logarithmic scale
  15. Connecting pH, pOH and Kw — Why pH plus pOH is fourteen only at 25 degrees Celsius
  16. One pH Unit Means a Tenfold Change — Comparing hydronium levels without treating pH as linear
  17. Neutral, Acidic and Basic at Different Temperatures — Classifying solutions by hydronium versus hydroxide
  18. pH of a Strong Monoprotic Acid — Using nearly complete ionisation under stated assumptions
  19. pH of a Strong Hydroxide Base — Counting hydroxide ions per formula unit
  20. Dilution and pH Change — Conserving solute amount before estimating pH
  21. Indicators and Their Color Ranges — Choosing a visual test that fits the pH question
  22. Universal Indicator and pH Paper — Estimating pH from calibrated color comparisons
  23. Using a pH Meter — Calibration, rinsing and what an electrode reads
  24. Acid–Base Neutralisation Equations — Writing molecular and net ionic descriptions
  25. Neutralisation Does Not Always Mean pH Seven — Distinguishing stoichiometric completion from neutral solution
  26. Acid–Base Mole Ratios — Counting transferable protons and hydroxide equivalents
  27. Titration as a Measurement of Amount — Converting an equivalence volume into unknown moles
  28. Titration Curves at an Introductory Level — Reading regions, equivalence and indicator suitability
  29. What a Salt Formula Represents — Balancing ionic charges in neutral salt units
  30. Preparing Salts by Acid–Base Reaction — Selecting reactants and separating dissolved product
  31. Preparing Salts with Metals or Carbonates — Recognising hydrogen or carbon dioxide alongside a salt
  32. Soluble and Insoluble Salts — Using solubility patterns to choose a preparation route
  33. Precipitation as Salt Preparation — Combining aqueous ions to isolate an insoluble product
  34. Crystallisation and Recovery of Soluble Salts — Concentrating a solution without decomposing its solute
  35. Salt Hydrolysis: The Central Idea — How a dissolved ion can react with water
  36. Salts of Strong Acid and Strong Base — Why some common salt solutions are approximately neutral
  37. Salts of Weak Acid and Strong Base — Basic anions formed from weak acids
  38. Salts of Strong Acid and Weak Base — Acidic cations formed from weak bases
  39. When Both Salt Ions Can Hydrolyse — Comparing competing acid and base tendencies qualitatively
  40. Sodium Chloride in Chemistry and Daily Life — Ionic composition, brine and practical uses
  41. Sodium Hydrogen Carbonate — Baking soda reactions with acid and heat
  42. Sodium Carbonate and Washing Soda — Carbonate chemistry, hydration and water-softening context
  43. The Chemistry of Water Hardness — Calcium and magnesium ions in domestic water
  44. How Carbonate Softens Hard Water — Precipitating calcium while accounting for solubility
  45. Bleaching Powder and Chlorine-Based Products — Composition, oxidising action and careful terminology
  46. Plaster of Paris and Gypsum — Calcium sulfate hydrates and reversible setting
  47. Acid Rain as Aqueous Chemistry — Formation and effects of sulfuric and nitric acid in precipitation
  48. Acids, Bases and Salts in Soil — Interpreting soil pH and responsible adjustment
  49. Choosing the Right Acid–Base Model — Comparing ionisation, proton transfer, pH and neutralisation claims
  50. pH and Salts: Integrated Review — Linking measurements, equations, calculations and practical uses